2B.1 lewis structure part b

[905290504]

hi guys!
for this question, you have to draw the lewis structure for COCl2. I was able to get the correct structure of carbon in the middle with single bonds to the two Cls and a double bond to oxygen. the Cls both have 3 lone pairs and the O has 2. I was wondering why we don't have resonance here. the answer manual only had this drawing, but couldn't we have a double bond between C and a Cl too (if we have a single bond for C-O)? why aren't there 3 resonance structures?

[Chem_Mod]

This is the most stable structure. If Cl were to have two bonds and then two lone pairs, its formal charge would be 7-(4+4/2) which equals +1.

[905290504]

also for part c you have to draw ONF and its O=N-F but why is the double bond with O if F is more electronegative?

[905290504]

This is the most stable structure. If Cl were to have two bonds and then two lone pairs, its formal charge would be 7-(4+4/2) which equals +1.

so when drawing structures, we should always just go with what gives us the most stable configuration regardless of the atom's electronegativity?

[Akash J 1J]

I don't believe electronegativity plays a role in determining whether the bond between atoms is single, double, or triple. Electronegativity primarily plays a part in determining the strength of a molecule's electric dipole moment.
And yes, you should generally go with what gives the most stable config. because atoms and molecules tend towards stability.

[Cooper_Geralds_3B]

This is the most stable structure. If Cl were to have two bonds and then two lone pairs, its formal charge would be 7-(4+4/2) which equals +1.

so when drawing structures, we should always just go with what gives us the most stable configuration regardless of the atom's electronegativity?

yes! Also though, if the question had asked about resonance structure- your answer would have been one correct answer. With lewis structure answers in the textbook they likely are just giving the most stable configuration, but definitely consider that there are often other correct answers.